The reaction of nitrogen dioxide and dinitrogen oxide results in the production of nitric oxide, NO, which is a potent greenhouse gas implicated in the depletion of ozone NO2(g) + N2O(g) -----à 3 NO ∆H = 155.67 kJ/mole ∆S = 171.4 J/moleK Find ∆G° for the reaction at 800 K and 1000 K; is the reaction spontaneous at either of these temperatures? Find the temperature at which the reaction becomes spontaneous under standard conditions.
The reaction of nitrogen dioxide and dinitrogen oxide results in the production of nitric oxide, NO, which is a potent greenhouse gas implicated in the depletion of ozone NO2(g) + N2O(g) -----à 3 NO ∆H = 155.67 kJ/mole ∆S = 171.4 J/moleK Find ∆G° for the reaction at 800 K and 1000 K; is the reaction spontaneous at either of these temperatures? Find the temperature at which the reaction becomes spontaneous under standard conditions.
Chemistry & Chemical Reactivity
10th Edition
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter18: Principles Of Chemical Reactivity: Entropy And Free Energy
Section: Chapter Questions
Problem 49PS
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- The reaction of nitrogen dioxide and dinitrogen oxide results in the production of nitric oxide, NO, which is a potent greenhouse gas implicated in the depletion of ozone
NO2(g) + N2O(g) -----à 3 NO ∆H = 155.67 kJ/mole ∆S = 171.4 J/moleK
Find ∆G° for the reaction at 800 K and 1000 K; is the reaction spontaneous at either of these temperatures? Find the temperature at which the reaction becomes spontaneous under standard conditions.
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